Matter and Measurement Flashcards

1
Q

is the field of study concerned with the characteristics, composition, and transformations of matter

A

Chemistry

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2
Q

includes all things, both living and non-living.

A

Matter

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3
Q

Physical state

A

Solid
Liquid
Gas

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4
Q

characterized by a definite shape and a definite volume

A

Solid

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5
Q

characterized by an indefinite shape and a define volume

A

Liquid

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6
Q

characterized by an indefinite shape and an indefinite volume

A

Gas

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7
Q

distinguishing characteristic of a substance that is used in its identification and description

A

Property

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8
Q

characteristics that can be observed without changing the basic identity of the substance (ex. Color, odor, physical state, melting/boiling point, hardness)

A

Physical property

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9
Q

describes the way the substance undergoes or resists change to form a new substance

A

Chemical property

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10
Q

a substance changes its physical appearance but not is chemical composition (ex. Changes in physical state)

A

Physical change

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11
Q

a substance undergoes a change in chemical composition. It always involve conversion of the material under consideration into one or more new substances

A

Chemical change

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12
Q

a single kind of matter that cannot be separated into other kinds of matter by any physical means

A

Pure substance

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13
Q

-physical combination of two or more pure substances in which each substance retains its own chemical identity
-One characteristic of any mixture is that its components can be separated using physical means

A

Mixture

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14
Q

a mixture that contains visible different phases (parts), each of which has different property

A

Heterogenous mixture

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15
Q

contains only one visibly distinct phase (part), which has a uniform properties throughout (ex. Sugar-water mixture)

A

Homogenous mixture

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16
Q

pure substance that cannot be broken down into simpler pure substances by chemical means

A

Element

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17
Q

pure substance that can broken down into two or more simpler pure substances by chemical means (ex. Water [H2O] can be broken down into the elements hydrogen and oxygen)

A

Compound

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18
Q

Notes: Compounds vs Mixtures
-Remember, substances can be combined either physically or chemically
-No such binding occurs during physical combination

A

Notes:
-Physical combination of substances produces a mixture
-Chemical combination of substances produces a compound, a substance in which combining entities are bound together

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19
Q

The discovery and isolation of the 117 known elements, the building blocks for all matter, have taken place over a period of several centuries. Most of the discoveries have occurred since

A

1700, the 1800s being the most active period

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20
Q

Note: Elements
Each element has a unique name; some bear geographical names (germanium, francium and polonium), some are named for the planets (mercury, uranium, neptunium), some reflect specific properties of the element or of the compounds containing it

A
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21
Q

one- or two-letter designation for an element derived from the element’s name

A

Chemical symbol

22
Q

is the smallest particle of an element that can exist and still have the properties of the element

23
Q

Note:
-A sample of any element is composed of atoms of a single type, those of that element. In contrast, a compound must have two or more types of atoms present, because by definition at least two elements must be present
-Free atoms are rarely encountered in nature
-Atoms are almost always found together in aggregates or clusters

24
Q

is a group of two or more atoms that functions a unit because the atoms are tightly bound together

25
is a molecule that contains two atoms, a triatomic molecule contains three, and so on.
diatomic molecule
26
is a molecule in which all atoms present are of the same kind. Substances containing (ex. Hydrogen [H2], oxygen [O2], nitrogen [N2], and chlorine [Cl2])
homoatomic molecule
27
is a molecule in which two or more kinds of atoms are present.
heteroatomic molecule
28
Note: -The atoms present may all be of the same kind, or two or more kinds may be present -Substances containing heteroatomic molecules are compounds (ex. Water [H2O]
29
molecules made of atoms from different elements
Compounds
30
atoms connected by chemical bond
Molecules
31
Note: ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS H2 is a molecule, but not a compound (only H is present) H2O is both a molecule and a compound (H and O are present)
32
is a notation made up of the chemical symbols of the elements present in a compound and numerical subscripts (located to the right of each chemical symbol) that indicate the number of atoms of each element present in a molecule of the compound.
chemical formula
33
determination of the dimensions, capacity, quantity, or extent of something
Measurement
34
Note: There are two systems of measurement that is used commonly: The English system of units and the metric system of units
35
Examples of units in the English system are
inch, foot, pound, quart, and gallon
36
Examples of units in the metric system are
gram, meter, and liter
37
Examples of units in the metric system are
gram, meter, and liter
38
Note: Metric System Units -In the metric system, there is one base unit for each type of measurement -Prefixes are then added to the base unit -The meter (m) is the base unit of length in the metric system (1 m is equivalent to 1.09 yards) -The gram (g) is the base unit of mass in the metric system (28 g = 1 ounce, 454 g = 1 pound) -The liter (L) is the base unit of volume in the metric system (1 L is equivalent to 1.06 quarts)
39
Measurements will always have a degree of uncertainty or error
Uncertainty in Measurements
40
are digits in a measurement that are known with certainty plus one digit that is estimated
Significant figures
41
are digits in a measurement that are known with certainty plus one digit that is estimated
Significant figures
42
note: -Uncertainty is indicated by the number of significant figures recorded -Number of significant figures = all certain digits + one estimated digit
43
. In multiplication and division, the number of significant figures
that contains the fewest significant figures
44
In addition and subtraction, the answer is given with as many significant figures as the measurement with the
least number of decimal places
45
is a numerical system in which numbers are expressed in the form A X 10n, where A is a number with a single nonzero digit to the left of the decimal place and n is a whole number
Scientific notation
46
Note: -The coefficients are combined in the usual way (multiplied or divided) -The rules for exponential terms are: 1. To multiply exponential terms, add the exponents 2. To divide the exponential terms, subtract the exponents Ex. (2.33 x 103) x (1.55 x 104) 2.33 x 1.55 = 3.61 103 x 104 = 103+4 = 107 Final answer is 3.61 x 107
47
is a ratio that specifies how one unit of measurement is related to another unit of measurement It is derived from equalities that relate units Ex. 1 minute = 60 seconds A pair of conversion factor can be derived from this equality (1 π‘šπ‘–π‘›π‘’π‘‘π‘’)/(60 π‘ π‘’π‘π‘œπ‘›π‘‘π‘ ) and (60 π‘ π‘’π‘π‘œπ‘›π‘‘π‘ )/(1 π‘šπ‘–π‘›π‘’π‘‘π‘’)
Conversion Factors
48
is a general problem-solving method in which the units associated with numbers are used as a guide in setting up calculations
Dimensional Analysis
49
-is the ratio of the mass of an object to the volume occupied by that object -Generally expressed in grams per cubic centimeter (g/cm3) for solids, grams per milliliters (g/mL) for liquids
π‘«π’†π’π’”π’Šπ’•π’š
50
π‘«π’†π’π’”π’Šπ’•π’š formula
π‘«π’†π’π’”π’Šπ’•π’š= π’Žπ’‚π’”π’”/π’—π’π’π’–π’Žπ’†
51
is a form of energy. Temperature is an indicator of the tendency of heat energy to be transferred
Heat
52
Note: -Heat energy flows from objects of higher temperature to objects of lower temperature. -Both the Celsius and the Kelvin are part of the metric system; Fahrenheit scale belongs to the English system -The Celsius scale is the most commonly used in scientific work